f. Which compounds will increase in amount as a result of this shift? (Enter "correct" for ALL correct answers.) • B • D g. Which compounds will decrease in amount as a result of this shift? (Enter "correct" for ALL correct answers.) • A • B • D h. When you heat the equilibrium mixture you notice that the concentration of compounds A and B increase and the concentration of compounds C and D decrease. In addition, you notice that when you cool the equilibrium mixture you notice that the concentration of compounds A and B decrease and the concentration of compounds C and D increase. You can add the "heat" term to the chemical equation to reflect these observations. Which chemical equation is correct? (Enter "correct for the correct equation.) A + B + heat C + D A + B > c +D+ heat

f. Which compounds will increase in amount as a result of this shift? (Enter "correct" for ALL correct answers.) • B • D g. Which compounds will decrease in amount as a result of this shift? (Enter "correct" for ALL correct answers.) • A • B • D h. When you heat the equilibrium mixture you notice that the concentration of compounds A and B increase and the concentration of compounds C and D decrease. In addition, you notice that when you cool the equilibrium mixture you notice that the concentration of compounds A and B decrease and the concentration of compounds C and D increase. You can add the "heat" term to the chemical equation to reflect these observations. Which chemical equation is correct? (Enter "correct for the correct equation.) A + B + heat C + D A + B > c +D+ heat

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

O KINETICS AND EQUILIBRIUM Calculating an equilibrium constant from a partial equilibrium... 0/5 Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 21. mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 6.3 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 II
NH3(g) + H2O(l) → NH2 + + H3O+ t The equilibrium constant is 1 x 10 -34. Is this reaction likely to take place? Why? Choose the best answer below. a. Yes, because the equilibrium constant is very small and equilibrium will lie far to the left. b. Yes, because the equilibrium constant is very small and equilibrium will lie far to the right. c. No, because the equilibrium constant is very small and equilibrium will lie far to the right. ☐ d. No, because the equilibrium constant is very small and equilibrium will lie far to the left. Click Submit to complete this assessment.
1) Decide whether each of the following statements is true or false. If false, change the wording of the statement to make it true. a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction. d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO (s) + Cao (s) + CO2 (g). e) For the reaction CaCO (s) + Cao (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.
Assume that the following endothermic chemical reaction is at equilibrium. C(s) + H₂O(g) + H₂(g) + CO(g) Which of the following statements is/are CORRECT? 1. Increasing the concentration of H₂(g) will cause the reaction to proceed in the backward direction, increasing the equilibrium concentration of H₂O(g). 2. Decreasing the temperature will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). 3. Increasing the amount of C(s) will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). All statements are correct. 2 only 3 only 1 only 1 & 2 only
3. Nitrogen gas and oxygen gas can combine to produce nitrogen monoxide. At 1500 K the equilibrium constant, Ke, is 1.0 x 10 . Suppose a sample of air has [N2] = 0.80 M and [O2] = 0.20 M before any reaction occurs. Calculate the equilibrium concentrations of product and reactants at equilibrium at this temperature.
d. Suppose you add compound E to the equilibrium mixture. Compound E reacts with compound D which is a component of the equilibrium to form compound F as described in the equation below. E + D Which compound is removed from the equilibrium mixture when you add compound E to the mixture? (Enter "correct" for ALL correct answers.) • B D e. What shift in the equilibrium will occur as a result of the addition of compound E? (Enter "correct" for the correct shift.) A + B C + D (shift to the right) A + B C + D (shift to the left)
Which of the following is true for chemical equilibrium? I. Forward and reverse reaction rates are equalII. Equilibrium can be achieved from either directionIII. Reaction rates and therefore equilibrium is temperature-dependent. a I only b I and II only c II and III only d I, II and III
For the chemical equation: SO2(g) + NO2(g) SO3(g) + NO(g) The equilibrium constant at a certain temperature is 8.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 6.20 mol SO2(g) in order to form 4.40 mol SO3(g) at equilibrium.
Suppose a reaction has a standard enthalpy change of -100 kJ. a) What temperature change would be needed to double the value of the equilibrium constant for this reaction? b) What temperature change would be needed to increase the value of the equilibrium constant for this reaction by a fact of ten? c) If the enthalpy change were only -20 kJ, what temperature change would be needed to double the value of the equilibrium constant for this reaction?
Use Le Châtelier’s Principle to explain the effect each of the following changes will have upon the system—will the equilibrium shift toward the product or reactant side? Why? N2(g) + 3 H2(g) ↔ 2 NH3(g) + heat a. If more hydrogen is added to the system the equilibrium will shift to the..... (pick one and explain)i. Right ii. Left iii. Remains unchanged b. If ammonia is removed from the system the equilibrium will shift to the..... (pick one and explain)i. Right ii. Left iii. Remains unchanged c. If nitrogen is removed from the system the equilibrium will shift to the..... (pick one and explain)
In an experiment, 1.000 mol H2 and 1.000 mol I2 are mixed in a 1.00-L container, and the reaction forms HI. If Kc = 54.3 for this reaction, what is the equilibrium concentration of HI? I2(g) + H2(g) ↔ 2HI(g) a. 1.572 b. 0.226 c. 0.399 d. 0.786 e. 0.899
A mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g) -> 2 SO3 At equilibrium, 0.0916 mol of SO3 is present. a. What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!) b. If the container size is 3.0 L, what is the value of the equilibrium constant?